Hybridization

Hybrid theory is a modification of atomic orbital
theory that was developed to explain the shapes of molecules. For example, a
tetrahedron cannot be formed if the only possible overlap of atoms is between
s, p or d orbitals, so we picture bonding orbitals in a tetrahedral molecule as
hybrids of s and p atomic orbitals that are oriented so they correspond to
molecular shapes.

Suggested
activity #1:

Since hybrid theory is so closely related to
molecular shape, this database can be used as practice of determining the types
of hybrids involved in various molecules. The "entry level" database would
probably be most useful since the molecular shape is clearer, but it could also
be interesting to try to predict what type of hybrids are found around each
atom of a some of the more complex structures. The different versions of the
databases will help regulate the complexity of the molecules being looked at.
For example, the entry level database will only deal with hybrids of s and p
orbitals, while the expanded valence database will keep the molecules fairly
simple but will include hybrids consisting of s, p and d orbitals.

Suggested
activity #2:

Hybrid orbitals possess a combination of the
characteristics of the component orbitals. For instance, an sp orbital
possesses half s character and half p character. A sp2 hybrid has
one third s character and two thirds p character. This idea can be conveyed by
looking at the relative lengths of various hybrid orbitals. We suggest
recording the bond lengths of a few sp, sp2 and sp3
molecules in a table to illustrate this phenomenon. Since a p orbital is longer
than an s orbital, the more p character in the hybrid, the longer the bonds
should be. (caution: compare molecules that are bonded to the same type of
orbital in the other atom. For instance, compare